Atomic structure and periodic table Flashcards

1
Q

What are elements?

A

An element is a substance that cannot be broken down into any other substance.

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2
Q

What are compounds?

A

Compounds are chemical substances made up of two or more elements that are chemically bound together.

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3
Q

What is a mixture?

A

A mixture is made when two or more substances are combined, but they are not combined chemically

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4
Q

What are separating techniques for mixtures?

A

Filtration (filter paper etc.)
Distillation (evaporating water and leaving solid)
Evaporation (evaporating water then leaving to cool to form crystals)

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5
Q

What is the difference between the plum-pudding model and the nuclear model?

A

Plum-pudding model = electrons in positively charged ‘soup’

Nuclear model = electrons orbit nucleus

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6
Q

What is the relative charge of protons neutrons and electrons?

A
Proton = +1
Neutron = 0
Electron = -1
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7
Q

What is the relative mass of protons, neutrons and electrons?

A
Proton = 1
Neutron = 1
Electron = 0
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8
Q

Which is the mass number and which is the atomic number?
23
NA
11

A
Mass number (top) = 23
Atomic number (bottom) = 11
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9
Q

How do you find the number of protons, neutrons and electrons from the atomic and mass number.

A
Protons = atomic number
Electrons = atomic number 
Neutrons = mass number - atomic number
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10
Q

What are isotopes?

A

Isotopes are members of a family of an element that all have the same number of protons but different numbers of neutrons.

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11
Q

What is relative atomic mass?

A

The relative atomic mass of an element is defined as the weight in grams of the number of atoms of the element contained in 12.00 g of carbon-12.

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12
Q

Why do isotopes affect the relative atomic mass?

A

The relative atomic mass of an element is a weighted average of the masses of the atoms of the isotopes - because if there is much more of one isotope then that will influence the average mass much more than the less abundant isotope will.

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13
Q

How do you find the relative atomic mass of an element given the abundance of its isotopes?

A
                       (percentage 1 + percentage 2)
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14
Q

How are elements in the periodic table arranged?

A

The chemical elements are arranged in order of increasing atomic number.

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15
Q

How are elements with similar properties placed in the periodic table?

A

Elements with similar properties are placed in vertical columns, called groups. elements in the same group have the same number of electrons in their outer shell.

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16
Q

Describe the early attempts to classify elements.

A

Early chemists attempted to classify the elements according to their relative atomic mass.

17
Q

Explain the creation and attributes of Mendeleev’s periodic table.

A

Mendeleev arranged the elements in order of increasing relative atomic mass. He then arranged the elements by putting those with similar properties below each other into groups.

18
Q

Describe noble gases (group 0) and explain their lack of reactivity.

A

When elements react, their atoms complete their outer shells by losing, gaining, or sharing electrons . The atoms of noble gases already have complete outer shells, so they have no tendency to lose, gain, or share electrons.

19
Q

What are the properties of noble gases?

A

Low boiling points.

Boiling point increases going down the group.

20
Q

Describe the reactivity and properties of alkali metals (group 1).

A

Reactivity increases down the group. This is because the outer electron in each atom is further away from the nucleus as you go down the group.

21
Q

Describe the properties of halogens (group 7).

A

The halogens have low melting points and low boiling points.
The halogens become darker as you go down the group.
Gas —> liquid —> solid as you go down the group
Get less reactive as you go down the group.

22
Q

Describe the reactions of halogens with metals and non-metals.

A

Halogen + metal —> salt

Halogen + hydrogen —> compound